Metals that can have multiple charges?

Calculate the concentrations of all species in a 1.21 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8.

Na

SO3

HSO3

H2SO3

OH

H

1.) Use a table of Standard Reduction Potentials to predict if a reaction will occur when Mg metal is put into a 1M aqueous H⁺solution.

If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank.

2.) Use a table of Standard Reduction Potentials to predict if a reaction will occur between Zn metal and I₂(s), when the two are brought in contact via standard half-cells in a voltaic cell.

If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank.

Ethyl alcohol has a vapor pressure of 20 mm Hg at 8 C and a normal boiling point of 78.4 C.
Estimate the vapor pressure at 45 C using (a) the Antoine equation
(b) the Clausius–Clapeyron equation and the two given data points; and (c) linear interpolation
between the two given points. Taking the first estimate to be correct, calculate the percentage error associated with the second and third estimates.

The Ka of a monoprotic weak acid is 7.85 × 10-3. What is the percent ionization of a 0.136 M solution of this acid?

Calculate the ratio of the energy released by the complete fission of 1.0 kg of Uranium-235 to the energy released by burning 1.0 kg of methane, CH4. You can use the fact that one mole of CH4 gives 802 kJ of energy, and recall from your chemistry course that there are 6.02*1023 atoms per mole.

How do you choose an appropiate indicator for a titration?

Why it is important to use such a small quantity of indicator in a titration?

What is the difference between the end point and equivalence point?

Can the End point be used quantitatively? why or why not?

If we rinse the buret with 33% NAOH solution instead of the 0.1M solution of NAOH and Water , How does this affect the result of our first trial? Assuming this is the only trial, how would this impact the calculated concentration of NaOH solution?

Calculate the anticipated pH for each of the solutions that resulted when you added HCl or NaOH to the "buffer" beaker. Enter the data in the tables below.

Buffer: (.100M NaC2H3O2 and .100M HC2H3O2) Concentration of both NaOH and HCl are .10M

Given the following equilibrium:

Br2 (g) + F2 (g) <----> 2 BrF (g)

Kc = 54.7 at 300 K

An evacuated flask is charged with 2.2 atm of Br2 and 2.2 atm of F2 at 300 K. Calculate the partial pressure of BrF at equilibrium at this temperature.

The IR spectra of the bis-dimedone derivative and the octahydroxanthenedione derivative should have significant differences in the frequency of the carbonyl stretch. Explain the reason for this difference.

Calculate the concentrations of all species in a 0.950 M Na2SO3 (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka1 = 1.4× 10–2 and Ka2 = 6.3× 10–8.

Physical Chemistry

hurricanes form when water vapor at the surface of the ocean(ca. 80 F) exchanges with the high altitude cooler air (ca. -120 F). During the ascent, the coriolis force of the earth creates massively destructive winds. in this sense, the hurricane is a heat engine whose upper bound on efficiency can be estimated from the second law. a typical hurricane condenses about 90 million tons of water per hour

a)Calculate the theoretical maximum efficiency of the hurricane, modeling the hurricane as a carnot engine

b)Modeling the hurricane as carnot engine, use the standard heat of vaporization for water to estimate the power output a hurricane can produce in W

1) When an abundance of amino acids occurs in the body, excess nitrogen has to be removed. OnewayinwhichthisisdoneisbyUreaSynthesis.

Part A: Describe the metabolic pathway in which Urea is produced, starting with free ammonium (NH4+) in the mitrochondria. What key intermediates are created? Which enzymes are needed to perform these transformations? How does this cycle relate to the TCA cycle?

Part B: Purines also need to be catabolized and removed from the body. What chemical form(s) does/do these purine-degradation product take? How to these products differ between species (e.g., mammals, birds, amphibians)?

Part C: Describe what happens when there are defects in the purine catabolic pathways. What sorts of diseases are a results the buildup of purine degradation products?

2) The energetics of glycolysis has been well studied. While the overall process is exergonic, very few of the steps are significantly so.

Part A: Describe those steps that are exergonic in detail. What sorts of chemical processesarehappening? Howwouldyouclassifyeachtypeofreaction?

Part B: Justify the exergonic nature of each of these steps. What is it about each step that leads to its spontaneous nature? Are any of these steps reversible? Why or why not? If not, how does the body overcome this lack of reversibility?

Part C: Overall, what do you think about the effectiveness and impact of energy generation (ATP generation) of anaerobic vs. aerobic catabolism? If one is more effective vs. the other, why do both types exist?

1. Consider the gas-phase reaction of PCl5, for which the equilibrium constant has the value of 11.5 at 300 degrees Celsius:

PCl5 (g) <---> PCl3 (g) +Cl2 (g)

a. Suppose enough PCl5 is placed in a flask of a certain volume at 300 degrees Celsius such that the initial pressure of PCl5 is 1.500 atm. Calculate the equilibrium pressure for each of the three gases, and also calculate the fraction of PCl5 that has dissociated to reach equilibrium. (If "x" is the amount that reacted, and "c" is the initial amount, then "x/c" is the fraction reacted.)

Ans: Equil Pressure PCl5______ PCl3_______ Cl2______ f=________

b. Now Suppose that 1.500 atm PCl5 is placed in a flask that also contains an initial pressure of 1.000 atm Cl2, with the initial pressure of PCl3=0. Calculate the equilibrium pressures, and the fraction related.

Ans: Equil pressure PCl5 ______ PCl3 ______ Cl2_______ f=________-

You are titrating 120.0 mL of 0.080 M Ca2+ with 0.080 M EDTA at pH 9.00. Log Kf for the Ca2+ -EDTA complex is 10.65, and the fraction of free EDTA in the Y4– form, αY4–, is 0.041 at pH 9.00.

(a) What is K'f, the conditional formation constant, for Ca2+ at pH 9.00?

(b) What is the equivalence volume, Ve, in milliliters?

(c) Calculate the concentration of Ca2 at V = 1/2 Ve.

(d) Calculate the concentration of Ca2 at V = Ve.

(e) Calculate the concentration of Ca2 at V = 1.1 Ve.